Nitrogen dioxide, , decomposes upon heating to form nitric oxide and oxygen according to the following equation: At the beginning of an experiment, the concentration of nitrogen dioxide in a reaction vessel was 0.1103 mol/L. After 64.0 s, the concentration decreased to 0.1054 mol/L. What is the average rate of decomposition of during this time interval in mol/(L·s)?

-7.66 x 10^-5 mol/L per second.

Explanation:

You find the avg. rate of decomposition by finding the overall amount of matter decomposed and dividing it by the time the mixture/substance decomposed for. In this case, it would be (0.1054 mol/L - 0.1103 mol/L ) / 64.0 s.

This gives you -0.0000766 mol/L per second (using significant figures rules), or -7.66 x 10^-5 mol/L per second.

Cheers.

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: