Give the relative rates for the following with a neighbor at your desk PH3(g) to P4(g)...

Question

Question

Give the relative rates for the following with a neighbor at your desk

PH3(g) to P4(g) + H2(g)

Remember to balance the equation

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Consider the reaction 4 PH3(g) → P4(g) + 6 H2(g). If, in a certain experiment, over...

Consider the reaction 4 PH3(g) → P4(g) + 6 H2(g). If, in a certain experiment, over a specific time period, 0.0045 mole of PH3 is consumed in a 1.7-L container during each second of the reaction, what are the rates of production of P4 and H2 in this experiment? P4 mol L−1 s−1 H2 mol L−1 s−1
Question 1 P4 (s) + 6 H2(g) → 4 PH3(g) What are the correct mole ratios...

Question 1 P4 (s) + 6 H2(g) → 4 PH3(g) What are the correct mole ratios based on the chemical equation above? BLANK-1 mol P4 : BLANK-2 mol PH3 BLANK-3 mol H2 : BLANK-4 mol PH3 BLANK-5 mol P4: BLANK-6 mol H2 BLANK-1 Add your answer BLANK-2 Add your answer BLANK-3 Add your answer BLANK-4 Add your answer BLANK-5 Add your answer BLANK-6 Add your answer
For the gas phase decomposition of phosphine at 120 °C 4 PH3(g)P4(g) + 6 H2(g) the...

For the gas phase decomposition of phosphine at 120 °C 4 PH3(g)P4(g) + 6 H2(g) the average rate of disappearance of PH3 over the time period from t = 0 s to t = 27 s is found to be 2.63×10-4 M s-1. The average rate of formation of H2 over the same time period is________ M s-1.

The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate...

The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate the activation energy, Eq, in kJ/mol for the reaction, given that the rate constant k (at 25 °C) = 0.00852 s 1 and k (at 50 °C) = 0.756 s 1. 231 kJ/mol 144 kJ/mol O 56.5 kJ/mol О 99.3 kJ/mol O 111 kJ/mol
The gas phase decomposition of phosphine at 120 °C PH3(g)1/4 P4(g) + 3/2 H2(g) is first...

The gas phase decomposition of phosphine at 120 °C PH3(g)1/4 P4(g) + 3/2 H2(g) is first order in PH3 with a rate constant of 1.80×10-2 s-1. If the initial concentration of PH3 is 5.86×10-2 M, the concentration of PH3 will be 1.43×10-2 M after s have passed.
The balanced equation P4 (s) + 6H2 (g) --> 4PH3 tells us that 2 mol H2 a

8. The balanced equation P4 (s) + 6H2 (g) --> 4PH3 tells us that 2 mol H2 a. reacts with 1 mol 4 b. produces 4 mol PH3 c. cannot react with phosphorus d. produces 2 mol PH3 e. reacts with 2 mol P4 idk y i cant seem to get the answer from the choices above?

The following data are for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4...

The following data are for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4 P4(g) + 3/2 H2(g) [ PH3 ], M 4.94×10-2 2.47×10-2 1.24×10-2 6.20×10-3 time, s 0 25.8 51.6 77.4 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is__ s . (2) Based on these data, the rate constant for this order reaction is__ s -1
2, Give the relative rates of disappearance of reactants and formation of products for each of...

2, Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. (a) 2 NO(g) +Br2(g) - 2 NOBr(g) (b) N2(g) + 3 H2(g) → 2 NH3(g) 3. In the reaction 2 03(g) → 3。2(g), the rate of formation of O2 is 1.5 x 10-3 molVL s. What is the rate of decom- position of 03? In the synthesis of ammonia, if-Δ[H21/Δt 4.5 × 10-4 mol/L-min, what is Δ[NH3VAt? N2(g) + 3 H2(g)...
Hess's Law Given the following data: P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0 kJ PH3(g) +...

Hess's Law Given the following data: P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0 kJ PH3(g) + 2O2(g) → H3PO4(l) ΔH°= -1272.0 kJ 2P(s) + 5/2O2(g) → P2O5(s) ΔH°= -1492.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°= -286.0 kJ calculate ΔH° for the reaction: H3PO4(l) → 1/2P2O5(s) + 3/2H2O(l) ΔH°=?? also please explain how you found the answer

the decomposition of phosphine forms phosphorus and hydrogen in the following reaction: 4PH3(g)--> P4(g)+6H2(g) A. express...

the decomposition of phosphine forms phosphorus and hydrogen in the following reaction: 4PH3(g)--> P4(g)+6H2(g) A. express the rate with respect to each of the reactants and oroducts. B. if the instantaneous rate with respect to PH3 is 0.34 M s^-1, what is the instantaneous rate of the reaction? use rate laws not calculus please.