**Chemical Reaction and Rate Problem****Reaction:** \[ 4 \text{PH}_3(g) \rightarrow \text{P}_4(g) + 6 \text{H}_2(g) \]**Problem Statement:** The average rate of consumption of \(\text{PH}_3\) is \(0.048 \, \text{M} \, \text{s}^{-1}\). Based on this average rate, what amount of \(\text{P}_4\) would be collected in 4.00 minutes in a 15.0 L container?**Options:** A. 173 moles B. 43.2 moles C. 86.4 moles D. 692 moles E. 346 moles **Explanation:**This is a stoichiometry problem involving a chemical reaction and the concept of reaction rates. Here, you are given the rate of consumption of one reactant and asked to calculate the amount of one of the products over a given time period in a specified volume. To solve:1. Calculate the total consumption of \(\text{PH}_3\) in moles over 4 minutes.2. Apply stoichiometry to determine how much \(\text{P}_4\) is formed from the consumed \(\text{PH}_3\).

Given question related to the calculation of the moles of phosphorus produced in the given reaction.

4PH3(g) →→→ P4(g) + 6H₂(g) -> The average rate of consumption of PH3 is 0.048 M s²¹. Based on this average rate, what amount of P4 would be collected in 4.00 minutes in a 15.0 L container? A. 173 moles B. 43.2 moles C. 86.4 moles D. 692 moles E. 346 moles

4PH3(g) →→→ P4(g) + 6H₂(g) -> The average rate of consumption of PH3 is 0.048 M s²¹. Based on this average rate, what amount of P4 would be collected in 4.00 minutes in a 15.0 L container? A. 173 moles B. 43.2 moles C. 86.4 moles D. 692 moles E. 346 moles

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the data from the previous question again. A--> B rate= 4.0 M/s B-->C rate = 1.5 M/min C-->D rate = 6.5 M/hour In the overall reaction A--> D, which step determines how fast the product D is made? a. C-->D b. B-->C c. A-->D d. A-->B
1. Below are 3 possible decompositions reactions for NaHCO3. Use stoichiometry to predict the percent mass lost as gases for each reaction. (Show all work, with units and stoichiometry) a. 2 NaHCO3(6) → 2 Na(s) + H2O2(e) + 2 CO2{@) b. 2 NaHCO3(5) → NazC2(s) + H2(e) + 3 O2(e) c. 2 NAHCO3(5) → NażCO3(s) + H2O8) + CO2(e)
I need help with 3,4, and 5.
Could you offer your expertise in solving these questions?
Remaining Time! 02:29:4. Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of Fe in the original mixture? Choose the closest answer. Fe(s) + 2 HCI(aq) FeCl2(aq) - + H2(g) 2 Al(s) +6 HC((aq) 2 AICI3(aq) + 3 H2(g) 96 % 69 % 47 % 33 % 17 % Rack Question Menu - O O
7. The rate of the endothermic reaction, H2CO3(aq)→H2O(l)+CO2(g), using 1.00 M H2CO3, can be increased by adding more water to the reactant boiling the water doubling the quantity of 1.00 M H2CO3 a. I only b. II only c. III only d. II and III only
Remaining Time: 1 hour, 01 minute, 47 seconds. * Question Completion Status: QUESTION 2 The number of water molecules in 2.3 mg of water is O 6.02 x 1023 O 77.0 x 1023 O 7.7 x 1023 O 7.7 x 1019 none of the above QUESTION 3 A ctudent makes a colution bu discolvina 254a ofNDOH int0 450 gof water Wh. Click Save and Submit to save and submit. Click Save All Answers to save all answer ere to search DELL
Please help me with all 'll Upvote you instantly please help me
In the reaction: 2NaOH(aq) + H2SO4(aq) → 2H2O(l) + Na2SO4(aq), what volume of 0.25 M NaOH would be needed to exactly react with 15 cm3 0.50 M H2SO4? Select one: a. 60 cm3 b. 15 cm3 c. 30 cm3 d. 7.5 cm3
a. b. C. d. e. 1. If for the reaction a b d e aX → by → 9 the rate law is determined to be r=[X]¹[Y]º the order of the reaction is 0 increasing the concentration of Y will have no effect on the rate increasing the concentration of X will have no effect on the rate increasing the concentration of Y will increase the rate of the reaction there is no way to determine the value of k 9 then
9. HCl (a strong acid) can dissolve Mg metal; if the rate of production of H₂ is 1.0x108 g H₂/s, find the mass of Mg consumed during 5.0 minutes (Hint: Watch your units on this one!) -5. 3.6×10'S
Enter your answer in the provided box. For the simple decomposition reaction AB(g)→ A(g) + B(g) rate = k[AB]2 and k = 0.10 L/mol·s. How long will it take for [AB] to reach 1/3 of its initial concentration of 1.50 M? t =_____s