At 600.0 k the rate constant is 6.1× 10–8 s–1. what is the value of the rate constant at 785.0 k?

1 answer:

5 0

Missing details. Complete text is:"The following reaction has an activation energy of 262 kJ/mol:
C4H8(g) --> 2C2h4(g)
At 600.0 K the rate constant is 6.1× 10–8 s–1. What is the value of the rate constant at 785.0 K?"
To solve the exercise, we can use Arrhenius equation:
$\ln( \frac{K_2}{K_1} ) = \frac{Ea}{R} ( \frac{1}{T_1}- \frac{1}{T_2} )$
where K are the reaction rates, Ea is the activation energy, R=8.314 J/mol*K and T are the temperatures. Using T1=600 K and T2=785 K, and Ea=262 kJ/mol = 262000 J/mol, on the right side of the equation we have
$\frac{Ea}{R}( \frac{1}{T_1}- \frac{1}{T_2} )=12.38$
And so
$\ln( \frac{K_2}{K_1})=12.38$
And using $K_1=6.1\cdot 10^{-8} s^{-1}$ , we find K2:
$K_2=K_1 e^{12.38}=0.0145 s^{-1}$

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2 years ago

A car travels a distance of 320 km in 4 hours. What is your average speed in meters per second?

Andreas93 [3]

Answer:

22.2 m/s

Explanation:

First, we need to convert km to m by multiplying by 1000. This means that the car traveled 320 000 meters.

Next, we convert hours to minutes by multiplying by 3600 (the number of seconds in an hour). This means that overall, the car traveled 320 000 m in 14 400 seconds.

The average speed can be found by using the equation $\frac{distance}{time}$ . After substitution, this gives the fraction $\frac{320 000}{14 400}$ , which reduces to 22 $\frac{2}{9}$ m/s, or about 22.2 m/s.