# You heat 0.158g of a white, solid carbonate of a Group 2 metal and find that the evolved #CO_2# has a pressure of 69.8 mmHg In a 285ml flask at 25°C .What is the molar mass of the metal carbonate?

The first step in this process is to calculate how many moles of carbon dioxide were produced by this decomposition reaction using the ideal gas law equation.

This is how the ideal gas law equation appears.

Now, it is crucial that you make sure you convert every unit you are given to the ones that the universal gas constant uses!

In this instance, you must convert the temperature from degrees Celsius to Kelvin, the volume from milliliters to liters, and the pressure from millibars to atm.

You'll get this

Currently, group 2 carbonates will decompose to produce carbon dioxide and metal oxide, so you can write

One mole of metal carbonate will have a mass of, since you know the mass of the sample. You can find the molar mass of the metal carbonate by dividing the mass of the sample by the number of moles that it contained.

Consequently, the metal's molar mass is

I'll round the result to four significant figures.

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The molar mass of the metal carbonate is approximately 98.2 g/mol.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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