Question

Consider the following reaction and associated information for Problems 2 and 3. 4 NH$_3$(g) + 5 O$_2$(g) $\longrightarrow$ 4 NO(g) + 6 H$_2$O(g) Rate = k[NH$_3$]$^2$[O$_2$]$^{1/2}$ 2. Which of the following is a correct representation of the relationship between the average rate of reaction and the concentration of chemicals? A. 4(rate) = $\frac{\Delta[NH_3]}{\Delta t}$ B. rate = $(\frac{1}{4})(\frac{\Delta[NH_3]}{\Delta t})$ C. 5(rate) = $-(\frac{\Delta[O_2]}{\Delta t})$ D. 4(rate) = $-\frac{\Delta[NO]}{\Delta t}$ E. rate = $-(\frac{1}{6})(\frac{\Delta[H_2O]}{\Delta t})$

          Consider the following reaction and associated information for Problems 2 and 3.
4 NH$_3$(g) + 5 O$_2$(g) $\longrightarrow$ 4 NO(g) + 6 H$_2$O(g)
Rate = k[NH$_3$]$^2$[O$_2$]$^{1/2}$
2. Which of the following is a correct representation of the relationship between the average rate of
reaction and the concentration of chemicals?
A. 4(rate) = $\frac{\Delta[NH_3]}{\Delta t}$
B. rate = $(\frac{1}{4})(\frac{\Delta[NH_3]}{\Delta t})$
C. 5(rate) = $-(\frac{\Delta[O_2]}{\Delta t})$
D. 4(rate) = $-\frac{\Delta[NO]}{\Delta t}$
E. rate = $-(\frac{1}{6})(\frac{\Delta[H_2O]}{\Delta t})$

Consider the following reaction and associated information for Problems 2 and 3.
4 NH3(g) + 5 O2(g) ⟶ 4 NO(g) + 6 H2O(g)
Rate = k[NH3]^2[O2]^1/2
2. Which of the following is a correct representation of the relationship between the average rate of
reaction and the concentration of chemicals?
A. 4(rate) = (Δ[NH3])/(Δ t)
B. rate = ((1)/(4))((Δ[NH3])/(Δ t))
C. 5(rate) = -((Δ[O2])/(Δ t))
D. 4(rate) = -(Δ[NO])/(Δ t)
E. rate = -((1)/(6))((Δ[H2O])/(Δ t))

Added by Elizabeth S.

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