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Chemistry

03/30/23

How many moles of C6H12 (cyclohexane) must be reacted according to the following balanced chemical reaction to transfer -419.1 kj of heat?

C₆H₁₂(l) + 9O₂(g)→ 6CO₂(g) + 6H₂O(g)∆H=-3919.4 kj-3919.4kJ

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Chemistry

03/30/23

What is the change in enthalpy when 1.50 moles of H2 are reacted with an excess O₂ of according to the following balanced chemical reaction: 2H₂(g)+O₂(g)→2H₂O(l) ∆H=-572 kj

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Chemistry

03/30/23

The steam reforming of methane occurs according to the following chemical equation:

CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g) Use the following equations to solve for the enthalpy change of steam reforming of methane: H₂(g) + ½O₂(g) → H₂O(g) ∆H° = -242 kJ/mol 2H₂(g) + C(s) → CH₄(g) ∆H°... more

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Chemistry

03/30/23

Using the equations

2 Fe (s) + 3 Cl₂ (g) → 2 FeCl₃ (s) ∆H° = -800.0 kJ/mol Si(s) + 2 Cl₂ (g) → SiCl₄ (s) ∆H° = -640.1 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃... more

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Chemistry

03/30/23

For the chemical reaction Ca (s) + ½ O₂ (g) → CaO (s) ∆H° = -635 kJ/mol. What is the molar enthalpy (in kJ/mol) for the reaction 2 CaO (s) → 2 Ca (s) + O₂ (g)?

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Chemistry

03/30/23

In the following reaction, what quantity in moles of CH₃OH are required to give off 1501 kJ of heat? 2 CH₃OH (l) + 3 O₂ (g) → 2 CO₂ (g) + 4 H₂O(g) ∆H° = -1280. kJ

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Chemistry

03/30/23

Determine the limiting reactant for the reaction, Calculate the mass of H3PO4 produced in the reaction, Calculate the percent yield of H3PO4 if 45.7 g H3PO4 is isolated.

A sample of 78.3 g78.3 g of tetraphosphorous decoxide (P4O10)(P4⁢O10) reacts with 78.1 g78.1 g of water to produce phosphoric acid (H3PO4)(H3⁢PO4) according to the following... more

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Chemistry

03/30/23

Combining 0.332 mol Fe2O3 with excess carbon produced 13.0 g Fe. Fe2O3+3C⟶2Fe+3CO What is the actual and theoretical yield of iron in moles?

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Chemistry

03/30/23

Potassium metal reacts with water according to the following balanced equation. 2K(s)+2H2O(l)⟶2KOH(aq)+H2(g) How many moles of KOH are produced if 2963.1 moles of H2O are consumed?

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Chemistry

03/30/23

Potassium metal reacts with water according to the following balanced equation. 2K(s)+2H2O(l)⟶2KOH(aq)+H2(g) How many moles of potassium are required to produce 18.0 moles of H2?

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Chemistry

03/30/23

How many grams of carbon dioxide ( CO2 ) are there in 1.27 mol of the compound?

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Chemistry

03/30/23

How many moles of potassium oxide (K2O) are in 77.5 g of the compound?

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Chemistry

03/29/23

ASAPStep by step having some trouble solving this

A given sample of gas has a volume of 4.20 L at 60 deg * C and standard pressure. Calculate its 70 / (27 deg) * C pressure, in atm, if the volume is changed to 5.00 L and the temperature . What we... more

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Chemistry

03/29/23

How much heat energy is needed to heat 200.0 g of water from 10.0 degrees C to 50.0 degrees C, with 4.184 J/g degreesC

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Chemistry

03/29/23

The balanced combustion reaction for C6H6 is 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ 2 ⁢ C 6 ⁢ H 6 ⁡ ( l ) + 15 ⁢ O 2 ⁡ ( g ) ⟶ 12 ⁢ CO 2 ⁢ ( g ) + 6 ⁢ H 2 O ( l ) + 6542 kJ

The balanced combustion reaction for C6H6 is2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJIf 6.600 g C6H6 is burned and the heat produced from the burning is added to 5691 g of water at 21 ∘C, what is... more

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Chemistry

03/29/23

A hot lump of 26.5 g of copper at an initial temperature of 77.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium.

A hot lump of 26.5 g of copper at an initial temperature of 77.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the... more

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Chemistry Math Science

03/29/23

Given the following enthalpies of formation, calculate the standard enthalpy change for the incomplete combustion of ethance (C2H6)

Reactants/Products ▲H fC2H6 -84.68 kJ/molO2 ... more

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Chemistry

03/29/23

Based on the sign of the standard cell potential, E°cell, classify these reactions as spontaneous or nonspontaneous as written

Based on the sign of the standard cell potential, E°cell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction... more

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Chemistry

03/29/23

What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode?

Consider these two entries from a fictional table of standard reduction potentials.X^3+ + 3e−⟶X(s) E°= −1.78 VY^3+ + 3e−⟶Y(s) E°= −0.23 VWhat is the standard potential of a galvanic (voltaic) cell... more

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Chemistry

03/29/23

Calculate the standard potential for this cell at 25∘C

A galvanic (voltaic) cell consists of an electrode composed of titanium in a 1.0 M titanium(II) ion solution and a second electrode composed of tin in a 1.0 M tin(II) ion solution, connected by a... more

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Chemistry

03/29/23

Calculate the standard potential for this cell at 25°C

A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M titanium(III) ion and 1.0 M titanium(II) ion, and another inert platinum electrode in a solution... more

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Chemistry

03/29/23

Calculate the standard potential for this cell at 25 °C

A galvanic (voltaic) cell consists of an electrode composed of zinc in a 1.0 M1.0 M zinc ion solution and another electrode composed of silver in a 1.0 M1.0 M silver ion solution, connected by a... more

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Chemistry

03/28/23

chemistry balanced equation

To obtain pure lead, lead (II) sulfide is burned in an atmosphere of pure oxygen. The products of the reaction are lead and sulfur trioxide (SO3). Write a balanced chemical equation for this process. more

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Chemistry

03/28/23

Asap step by step I did try solving this and I got 4.1 which is wrong so if you could tell me what I did wrong

If 10 g of oxygen gas is in a 2.00 L container at 50 Cwhat is the pressure in the container ? Round to one decimal place. Don’t forget oxygen is diatomic

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Chemistry

03/28/23

ASAP Step by step I really am not understanding how to solve this problem

If 10 g of oxygen gas is in a 2.00 L container at 50 Cwhat is the pressure in the container ? Round to one decimal place.When the temperature of a rigid hollow sphere containing 685 L of helium gas... more

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How many moles of C6H12 (cyclohexane) must be reacted according to the following balanced chemical reaction to transfer -419.1 kj of heat?

What is the change in enthalpy when 1.50 moles of H2 are reacted with an excess O₂ of according to the following balanced chemical reaction: 2H₂(g)+O₂(g)→2H₂O(l) ∆H=-572 kj

The steam reforming of methane occurs according to the following chemical equation:

Using the equations

For the chemical reaction Ca (s) + ½ O₂ (g) → CaO (s) ∆H° = -635 kJ/mol. What is the molar enthalpy (in kJ/mol) for the reaction 2 CaO (s) → 2 Ca (s) + O₂ (g)?

In the following reaction, what quantity in moles of CH₃OH are required to give off 1501 kJ of heat? 2 CH₃OH (l) + 3 O₂ (g) → 2 CO₂ (g) + 4 H₂O(g) ∆H° = -1280. kJ

Determine the limiting reactant for the reaction, Calculate the mass of H3PO4 produced in the reaction, Calculate the percent yield of H3PO4 if 45.7 g H3PO4 is isolated.

Combining 0.332 mol Fe2O3 with excess carbon produced 13.0 g Fe. Fe2O3+3C⟶2Fe+3CO What is the actual and theoretical yield of iron in moles?

Potassium metal reacts with water according to the following balanced equation. 2K(s)+2H2O(l)⟶2KOH(aq)+H2(g) How many moles of KOH are produced if 2963.1 moles of H2O are consumed?

Potassium metal reacts with water according to the following balanced equation. 2K(s)+2H2O(l)⟶2KOH(aq)+H2(g) How many moles of potassium are required to produce 18.0 moles of H2?

How many grams of carbon dioxide ( CO2 ) are there in 1.27 mol of the compound?

How many moles of potassium oxide (K2O) are in 77.5 g of the compound?

ASAPStep by step having some trouble solving this

How much heat energy is needed to heat 200.0 g of water from 10.0 degrees C to 50.0 degrees C, with 4.184 J/g degreesC

The balanced combustion reaction for C6H6 is 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ 2 ⁢ C 6 ⁢ H 6 ⁡ ( l ) + 15 ⁢ O 2 ⁡ ( g ) ⟶ 12 ⁢ CO 2 ⁢ ( g ) + 6 ⁢ H 2 O ( l ) + 6542 kJ

A hot lump of 26.5 g of copper at an initial temperature of 77.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium.

Given the following enthalpies of formation, calculate the standard enthalpy change for the incomplete combustion of ethance (C2H6)

Based on the sign of the standard cell potential, E°cell, classify these reactions as spontaneous or nonspontaneous as written

What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode?

Calculate the standard potential for this cell at 25∘C

Calculate the standard potential for this cell at 25°C

Calculate the standard potential for this cell at 25 °C

chemistry balanced equation

Asap step by step I did try solving this and I got 4.1 which is wrong so if you could tell me what I did wrong

ASAP Step by step I really am not understanding how to solve this problem

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