Ethyne gas combusts with oxygen gas according to the following reaction: calculate the volume, in ml of co2 produced when 73 g of c2h2 react at 37.4 °c and 1.6 atm. (r = 0.08206 l atm/mol k) latex: 2\: c_2h_2\left(g\right)\: +\: 5o_2\left(g\right)\: \longrightarrow\: 4\: co_2\left(g\right)\: +2\: h_2o\left(l\right)\:

Volume of CO2 is 89127 mL

Explanation: The reaction that takes place is: C2H2 + O2 --> CO2 + H2O

The amount of C2H2 that react allow us to predict the amount of CO2 that will be obtained

26g/1mol is molar mass of C2H2 and 2/4 is the molar relation between CO2 and C2H2 in this reaction. Canceling units, at the end mol of CO2 are obtained

Now with the moles of CO2 and the ideal gases equation is possible to calculate the volumen occupied by the gas.

PV = RnT where P: pressure, V: volume, R: ideal gas constant, n: moles and T: temperature expressed in K (add 273,15 to °C temperature: 37,4°C + 273,15 = 310,55K)

V= RnT/P

To express volume in mL multiply the L result by 1000 which equals 89127 mL

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.