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 3 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 equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g)...

The equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? equilibrium, left, right? PNO2 = 0.154 atm, PN2O4 = 0.148 atm...

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