By analyzing the data, it is clear that if we double the concentration of A keeping congratulation of B constant, rate remains same. It means order of reaction with respect to A is zero.
And if we double the concentration of B keeping concentration of A constant, rate of reaction becomes 4 times. It means order of reaction with respect to B is two.
Using the information in the table, the value of the rate constant for the reaction A(g)...
| Metro by T-Mobile 10:41 AM Time's Up! View Feedback Using the information in the table, the value of the rate constant for the reaction 2 A(g) + B(g) → C(g) + D(g) is [A]. (M) [B]. (M) Rate (M/min) 0.150 0.300 3.38 x 10-5 0.450 0.300 1.01 x 10-4 0.450 0.150 2.54 x 10-5 A) 0.00250 M-2min-1 Tap here or pull up for additional resources
Using the data in the table, calculate the rate constant of this reaction. Trial [A] (M) 0.360 0.360 0.612 [B] (M) 0.380 1.03 0.380 Rate (M/s) 0.0230 0.168 0.0391 A+B C +D 3 Units k=
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A + 2 B ⟶ C + D Trial [ A ] (M) [ B ] (M) Rate (M/s) 1 0.270 0.360 0.0182 2 0.270 0.720 0.0182 3 0.540 0.360 0.0728 k = Units=
Using the data in the table, calculate the rate constant of this reaction. Trial[ A(M)[B(M)Rate (M//s)10.3000.3900.017620.3000.8970.093130.4800.3900.0282A+B → C+D
Using the data in the table, calculate the rate constant of this reaction. TrialA(M)B(M)Rate (M//s)10.3000.2600.019920.3000.7280.15630.3900.2600.0259A+B → C +D k = _______
1. Initial‑rate data at a certain temperature is given in the table for the reaction N2O3(g)⟶NO(g)+NO2(g) [N2O3]0(M) Initial rate (M/s) 0.100 0.510 0.200 1.020 0.300 1.530 Determine the value and units of the rate constant. k= units: 2. Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [A] (M)[A] (M) [B] (M)[B] (M) Rate (M/s) 1 0.340 0.340 0.0127 2 0.340 0.680 0.0127 3 0.680 0.340 0.0508 k= Units...
QUESTION 1QUESTION 2 QUESTION 3 Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units 1 0.270 0.270 0.0110 2 0.270 0.0110 0.540 A + 2 B C + D 0.270 0.540 0.0440 Units k = Using the data in the table, calculate the rate constant of Rate (M/s) Trial [A] (M) [B] (M) this reaction 1 0.360 0.0222 0.320 2 0.360 0.704 0.107 А...
2. Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [A] (M)[A] (M) [B] (M)[B] (M) Rate (M/s) 1 0.340 0.340 0.0127 2 0.340 0.680 0.0127 3 0.680 0.340 0.0508 k= Units 3. The rate constant for this first‑order reaction is 0.480 s−1 at 400 ∘C. A⟶products How long, in seconds, would it take for the concentration of A to decrease from 0.650 M to 0.270 M? 4. After...
The rate constant for the gaseous reaction H2(g) + I2(g) → 2HI(g) is 2.42 × 10−2/(M·s) at 400°C. Initially an equimolar sample of H2 and I2 is placed in a vessel at 400°C and the total pressure is 1690 mmHg. (a) What is the initial rate (M·min) of formation of HI? (__________) (b) What are the rate of formation of HI and the concentration of HI (in molarity) after 13.4 min? Rate of formation = (_______) (c) [HI] = (_______)...
Use the table below to solve for the rate constant for the reaction A + 2B + 2C - products. Trial [A], M 0.420 1 [B],M 0.150 0.150 [C],M Initial rate, M/s 0.330 4.00 0.330 4.00 2 0.210 3 0.420 0.225 0.330 6.00 4 0.420 0.150 0.660 8.00 Type in a numerical answer only with the correct sig figs. Do NOT type in units.