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Varvara68 [4.7K]
3 years ago
13

What’s the mass of 2.80 mol of ca

Chemistry
1 answer:
Ludmilka [50]3 years ago
3 0

Answer:

112.22 g

Explanation:

mass = no. of moles x atomic mass

From the periodic table, we can see the atomic mass of Ca is 40.078.

Therefore,

mass = 2.80 x 40.078

= 112.22g (corrected to 2 decimal places.)

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Determine the mass of CaCO3 required to produce 40.0 mL CO2 at STP. Hint use molar volume of an ideal gas (22.4 L)
cupoosta [38]

Answer:

m_{CaCO_3}=0.179gCaCO_3

Explanation:

Hello,

In this case, since the undergoing chemical reaction is:

CaCO_3(s)\rightarrow CaO(s)+CO_2(g)

The corresponding moles of carbon dioxide occupying 40.0 mL (0.0400 L) are computed by using the ideal gas equation at 273.15 K and 1.00 atm (STP) as follows:

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Then, since the mole ratio between carbon dioxide and calcium carbonate is 1:1 and the molar mass of the reactant is 100 g/mol, the mass that yields such volume turns out:

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Regards.

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