Consider this reaction:→2H3PO4aq+P2O5aq3H2OaqAt a certain temperature it obeys this rate law.rate =·1.68M−1s−1H3PO42Suppose a vessel contains H3PO4 at a concentration of 0.850M. Calculate the concentration of H3PO4 in the vessel 4.30 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.
Question
Consider this reaction:→2H3PO4aq+P2O5aq3H2OaqAt a certain temperature it obeys this rate law.rate =·1.68M−1s−1H3PO42Suppose a vessel contains H3PO4 at a concentration of 0.850M. Calculate the concentration of H3PO4 in the vessel 4.30 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.
Solution
The given rate law is: rate = k[H3PO4]^2
Where: k = 1.68 M^-1s^-1 (rate constant) [H3PO4] = concentration of H3PO4
The rate of reaction is also given by the change in concentration over the change in time:
rate = -Δ[H3PO4]/Δt
We can set these two expressions for the rate equal to each other and solve for the change in concentration:
-Δ[H3PO4]/Δt = k[H3PO4]^2
Rearranging to solve for Δ[H3PO4] gives:
Δ[H3PO4] = -k[H3PO4]^2 * Δt
Substituting the given values:
Δ[H3PO4] = -(1.68 M^-1s^-1)(0.850 M)^2 * 4.30 s
Calculate the above expression to find the change in concentration. Then subtract this value from the initial concentration to find the final concentration of H3PO4. Round your answer to 2 significant digits.
Similar Questions
A chemistry graduate student is studying the rate of this reaction:→2H3PO4aq+P2O5aq3H2OaqShe fills a reaction vessel with H3PO4 and measures its concentration as the reaction proceeds:time(milliseconds) H3PO40 0.500M10. 0.219M20. 0.140M30. 0.103M40. 0.0817MUse this data to answer the following questions.Write the rate law for this reaction. rate =k Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. =k
At a certain temperature the rate of this reaction is first order in N2O5 with a rate constant of 4.96s−1:→2N2O5g+2N2O4gO2gSuppose a vessel contains N2O5 at a concentration of 0.530M. Calculate the concentration of N2O5 in the vessel 0.150 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.
Consider this reaction:→2NH3g+N2g3H2gAt a certain temperature it obeys this rate law.rate =2.89s−1NH3Suppose a vessel contains NH3 at a concentration of 0.640M. Calculate the concentration of NH3 in the vessel 0.380 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.
At a certain temperature this reaction follows second-order kinetics with a rate constant of ·0.0577M−1s−1:→NH4OHaq+NH3aqH2OaqSuppose a vessel contains NH4OH at a concentration of 1.16M. Calculate the concentration of NH4OH in the vessel 53.0 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.M
A chemistry graduate student is studying the rate of this reaction:→NH4OHaq+NH3aqH2OaqShe fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds:time(seconds) NH4OH0 0.400M1.0 0.277M2.0 0.191M3.0 0.132M4.0 0.0915MUse this data to answer the following questions.Write the rate law for this reaction. rate=k Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.