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Which change will cause a change in the equilibrium constant? SiF4(g) + 2H2O(g) ⇌ SiO2(s) + 4HF(g) ∆Ho = +148.9kJ

Adding more SiO2(s)
B. Increasing the temperature
C. Decreasing the pressure by increasing the volume
D. Removing water

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Which of the following can NOT reach the equilibrium shown by the equation CaCO3(s) ⇌ CaO(s) + CO2(g)

A. Pure CaCO3(s)
B. Pure CaO(s)
C. A mixture of CaCO3(s) and CaO(s)
D. CaO(s) and a concentration of CO2(g) greater than the equilibrium concentration

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For a given reaction, doubling the temperature will increase the reaction rate by ()

A. 2
B. 0.61
C. 2.7
D. 1.6

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The reaction C ® products is a first-order reaction with t1/2 = 1.3 ´ 104 s. If the initial concentration of C is 0.200 M, what will be the concentration of C after 2.6 ´ 104 s? ( )

A. 0.025 M
B. 0.050 M
C. 0.100 M
D. 0.200 M

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The rate law for a reaction B ® products is rate = k[B], which graph will give a straight line? ( )

A. ln[B] vs. time
B. [B] vs. time
C. 1/[B] vs. time
D. ln[B] vs. 1/time

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Which change will cause a change in the equilibrium constant? SiF4(g) + 2H2O(g) ⇌ SiO2(s) + 4HF(g) ∆Ho = +148.9kJ

Adding more SiO2(s) B. Increasing the temperature C. Decreasing the pressure by increasing the volume D. Removing water

Which of the following can NOT reach the equilibrium shown by the equation CaCO3(s) ⇌ CaO(s) + CO2(g)

For a given reaction, doubling the temperature will increase the reaction rate by ()

The reaction C ® products is a first-order reaction with t1/2 = 1.3 ´ 104 s. If the initial concentration of C is 0.200 M, what will be the concentration of C after 2.6 ´ 104 s? ( )

The rate law for a reaction B ® products is rate = k[B], which graph will give a straight line? ( )

Adding more SiO2(s)
B. Increasing the temperature
C. Decreasing the pressure by increasing the volume
D. Removing water