03/23/23

Calculate the activation energy, 𝐸a�a, in kilojoules per mole for a reaction at 70.0⁢ ∘C that has a rate constant of 0.272⁢ s−1 and a frequency factor of 1.18×1011 s−1.
Calculate the activation energy, 𝐸a�a, in kilojoules per mole for a reaction at 70.0⁢ ∘C that has a rate constant of 0.272⁢ s−1 and a frequency factor of 1.18×1011 s−1.𝐸a=�a=kJ/mol
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03/23/23

The rate constant for this first-order reaction is 0.0235 s−1 at 300 °C.
The rate constant for this first-order reaction is 0.0235 s−1 at 300 °C. A⟶productsIf the initial mass of A is 19.02 g, calculate the mass of A remaining after 1.41 min.mass of A: g
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03/23/23

The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 475 K is 0.0450 1/min, then what is the value of the rate constant at 789 K? (R = 8.314 J/mol • K)
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03/23/23

A 165.0 mL solution of 2.282 M strontium nitrate is mixed with 220.0 mL of a 2.278 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate.
Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration.Find Na+NO-3Sr2F-
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03/22/23

Determine the limiting reagent of MgO(s)+2HCl(aq)= MgCl2(aq)+H2O when there are 1.0g MgO and 76.3g HCl
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03/22/23

Determine the limiting reagent in Mg(s)+2HCl(aq)= MgCl2(aq)+H2(g) when Mg has .122g and HCl has 40.68g
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03/22/23

Determine the limiting reagent in Mg(s)+2HCl(aq)= MgCl2(aq)+H2(g)
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03/22/23

If 50 ml of water at 85 degrees C are added to 100ml of water at 25 degrees C what would be the final temperature of the water assuming that no heat is lost to surroundings?
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03/22/23

Determine the molecular weight of the vapour.
A 256.0 cm^3 flask is filled with a vapour at 97.325 KPa and 100 C. The mass of the vapour is 1.675 g. Determine the molecular weight of the vapour. Use R = 8.314 JK^-1mol^-1.
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03/22/23

Determine the formula of the hydrate.
A hydrate of barium chloride, BaCl2nH2O, weighing 1.222 g was heated until all the combined water was expelled. The dry powder remaining weighed 1.042 g.Determine the formula of the hydrate.
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03/22/23

Calculate the percentage elemental composition of the confiscated substance.
A white substance had been confiscated on suspicion that it was cocaine. A forensic chemist purified the substance and subjected it to elemental analysis. Combustion of a 50.86 mg sample yielded... more
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03/22/23

A student collects 500 cm^3 of methane gas at STP. Determine the moles of gas present, the number of methane molecules and the mass of methane.
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03/21/23

pH of the solution

A solution contains 0.228 M C2H5NH3Br and 0.126 M ethylamine , C2H5NH2 .What is the pH?
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03/21/23

Identify the reactant that gets oxidized in the following reaction. 2Al(s) + 6HCl(aq) → 2AlCl₃(aq) + 3H₂(g)
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03/21/23

chemistry 11 grade
0.465 mole sample of gas everts 4.43 atm of pressure in a 2.25 L container. What is temperature of the gas un the container ?
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03/21/23

Equilibrium Shift
4 NH3(g) + 5 O2(g) ↔ 4 NO(g) + 6 H2O(g) ΔH = -904.4 kJ How does each of the following changes affect the yield of NO at equilibrium? Answer increase, decrease, or no change: a) increase [NH3]; b)... more
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03/21/23

Equilibrium Constant
Consider the reaction: SO2Cl2(g) ↔ SO2(g) + Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of 0.020M. At equilibrium, [Cl2] = 1.2x10-2M. Calculate the value of the equilibrium... more
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03/21/23

Equilibrium constant
Use the following reactions and their equilibrium constants to predict the equilibrium constant for this reaction: 2 A(s) ↔ 3 D(g).A(s) ↔ 1⁄2 B(g) + C(g) K1 = 0.03343D(g)↔B(g)+2C(g) K2 =2.35
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03/21/23

Equilibrium questions
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(g) + Cl2(g) ↔ PCl5(g). A 7.5L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is... more
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03/21/23

Calculate equilibria constant
The following equilibria were attained at 823K: CoO(s) + H2(g) ↔ Co(s) + H2O(g) CoO(s) + CO(g) ↔ Co(s) + CO2(g) Based on these equilibria, calculate the equilibrium constant for H2(g) + CO2(g) ↔... more
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03/21/23

Calculate the H3O + concentration at the halfway point when 38.8 mL of 0.15 M HBr is titrated with 0.1 M KOH. Assume additive volumes. Answer in units of M
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03/20/23

Equilibrium and using ICE tables
Solid Ca₃(PO₄)₂ is placed into 10.0 L of water. When equilibrium is established, the concentration of Ca²⁺ is 2.3 × 10⁻⁴ M. What is Kc for this equilibrium? Note Kc is sometimes called K. Ca₃(PO₄)₂... more
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03/20/23

Equilibrium and using ICE tables
For the reaction below, Kc = 1.10 × 10⁻⁴. Note Kc is sometimes called K. What is the equilibrium concentration of C if the reaction begins with 0.200 M A and 0.400 M B? 2 A (aq) + B (aq) ⇌ C (aq)
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03/20/23

Equilibrium and using ICE tables
An empty steel container is filled with 0.0400 atm of HF. The system is allowed to reach equilibrium. If Kp = 2.76 for the reaction below, what is the equilibrium partial pressure of H₂? 2 HF (g) ⇌... more
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03/20/23

Consider the titration of 30.0 mL of 0.251 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. What is the pH of the solution at the equivalence point?
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