A 1.00 L volume of dry air is sealed inside of a round flask and brought to a temperature of 50.0°C in a hot water bath. If the pressure gauge reads 3.60 atm, how many moles of gas are in the sample of

air?

0.136mol

Explanation:

Using the general gas law equation as follows:

PV = nRT

Where;

P = pressure (atm)

V = volume (Litres)

n = number of moles (mol)

R = gas constant (0.0821 Latm/mol K)

T = temperature (K)

K = °C + 273

K = 50°C + 273

K = 323K

According to this question, P = 3.6atm, T = 323K, V = 1.00L, R = 0.0821 Latm/mol K, n = ?

3.6 × 1 = n × 0.0821 × 323

3.6 = 26.52n

n = 3.6/25.52

n = 0.1357

n = 0.136mol

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: