The mass of the water is 1580 g.
<h3>What is the amount of water formed?</h3>
We know that the ideal gas equation can be used to obtain the number of moles of the gas. We have been told that the pressure of the gas reduced from 7.9 x 10-3 atm to 1.2 x 10-4 atm. The change in pressure can be used obtain the number of moles.
Change in pressure = 7.9 x 10-3 - 1.2 x 10-4 = 7.78 * 10^-3 atm
Using;
PV = nRT
n = PV/RT
n = 7.78 * 10^-3 atm * 2.4 x10^5 l/0.082 * (39 + 273)
n = 85 moles
Since 1 mole of carbon dioxide produces 1 mole of water
85 moles of carbon dioxide produces 85 mole of water
Mass of water produced = 85 mole * 18 g/mol
= 1580 g
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Answer:
Explanation:
Hello.
In this case, given the chemical reaction, we can compute the grams of oxygen by using the 98.2 g of water via the 2:1 mole ratio between them, the molar mass of water that is 18.02 g/mol, the molar mass of gaseous oxygen that is 32.00 g/mol and the following stoichiometric procedure relating the given information:
In which the result is displayed with three significant figures because the given mass of water 98.2 g, has three significant figures too.
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Answer:
answer is
Explanation:
Gallium because it has the properties which you have mentioned
