The half-life for the first-order decomposition of N2O4 is 1.3×10?5s. N2O4(g)?2NO2(g) Part A If N2O4 is...

The half-life for the first-order decomposition of N2O4 is 1.3×10?5s. N2O4(g)?2NO2(g) Part A If N2O4 is introduced into an evacuated flask at a pressure of 19.0 mmHg, how many seconds are required for the pressure of NO2 to reach 1.4 mmHg?

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queen_honey_blossom answered 2 years ago

The half-life for the first-order decomposition of N204is 1.3 x 10-5s N2O4 (g) arrow sign 2NO2(g)...

The half-life for the first-order decomposition of N204is 1.3 x 10-5s N2O4 (g) arrow sign 2NO2(g) If N204is introduced into an evacuated flask at a pressure of 17.0 mm Hg, how many seconds are required for the pressure of NO2 to reach 1.3 mm Hg? What is the value of the rate constant?_____/second (2 s.f.) What is the elapsed time for the reaction? _____seconds (2 s.f.) use E to express powers of ten, i.e. 6.02x1023 =6.02E23 Please fill in the...

The half-life for the first-order of decomposition is 1.3 x 10^-5s N2O4(g) 2N02(g) If N2O4 is...

The half-life for the first-order of decomposition is 1.3 x 10^-5s N2O4(g) 2N02(g) If N2O4 is introduced into an evacuated flask at a rate of 17.0mm Hg, how many seconds are required for the No2 to reach 1.3 mm Hg? To solve this problem one plots a graph of______ versus _____. the slope of this lie is equal to negative activation energy divided by ______and has the value ______ 104 K. (2 s.f.) The activation energy is ______ kJ/mole (2...

N2O4 (g) ⇌ 2NO2(g). KP = 0.10 at some Temperature. If 0.40 atm of N2O4 is...

N2O4 (g) ⇌ 2NO2(g). KP = 0.10 at some Temperature. If 0.40 atm of N2O4 is placed in an evacuated flask, what are the pressures at equilibrium?

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a...

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K? [N2O4], [NO2] =

The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If...

The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If a reaction vessel at that temperature initially contains 0.030M NO2 and 0.030M N2O4, what are the concentrations of the two gases at equilibrium? First, the reaction quotient (Q) [page 645 of textbook] must be calculated, and then use the I.C.E table [page 648-650 of the textbook] to determine the equilibrium concentrations.

Exercise 14.80 The half-life for the first-order decomposition of nitramide, NH2NO2(aq)→N2O(g)+H2O(l), is 123 min at 15∘C....

Exercise 14.80 The half-life for the first-order decomposition of nitramide, NH2NO2(aq)→N2O(g)+H2O(l), is 123 min at 15∘C. Part A If 170 mL of a 0.105 M NH2NO2 solution is allowed to decompose, how long must the reaction proceed to yield 46.0 mL of N2O(g) collected over water at 15∘C and a barometric pressure of 756 mmHg ? (The vapor pressure of water at 15∘C is 12.8 mmHg.) Express your answer using two significant figures. t = min Please show as much...

At –80°C, K for the reaction N2O4(g) 2NO2(g) is 4.66 × 10–8. We introduce 0.049 mole...

At –80°C, K for the reaction N2O4(g) 2NO2(g) is 4.66 × 10–8. We introduce 0.049 mole of N2O4 into a 1.0-L vessel at –80°C and let equilibrium be established. The total pressure in the system at equilibrium will be: (0.78 atm)

Part A What is the half-life of a first-order reaction with a rate constant of 1.80×10−4 s−1?...

Part A What is the half-life of a first-order reaction with a rate constant of 1.80×10−4 s−1? Express your answer with the appropriate units. Part B What is the rate constant of a first-order reaction that takes 163 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. Part C A certain first-order reaction has a rate constant of 3.10×10−3 s−1. How long will it take for the reactant concentration to...

The degree of dissociation, α, for the following reaction: N2O4(g) <--> 2NO2(g) is 0.655 at 298...

The degree of dissociation, α, for the following reaction: N2O4(g) <--> 2NO2(g) is 0.655 at 298 K and 1.00 bar total pressure. Find K.

The decomposition of N2O5(g) —> NO2(g) + NO3(g) proceeds as a first order reaction with a...

The decomposition of N2O5(g) —> NO2(g) + NO3(g) proceeds as a first order reaction with a half life 30.0s at a certain temperature. If the initial concentration [N2O5]0 = 0.400 M, what is the concentration after 120 seconds? A)0.050 B)0.200 C)0.025 D)0.100

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