Answer:

Explanation:
Hello,
In this case, since the law of conservation of mass allows us to notice that the mass of carbon in the burned compound is also present in the resulting carbon dioxide, we can compute such moles as shown below:

Next, hydrogen in the sample is present at the products in the water only, and in one mole of water, two moles of hydrogen are present, thereby:

Nevertheless, the amount of oxygen in the sample must be computed by subtracting both the mass of carbon and hydrogen from the previously computed moles:

And the moles:

Next, we compute the mole ratios with respect to the element having the smallest number of moles (oxygen) to obtain the subscripts in the empirical formula:

Then, we have:

Finally, by multiplying by two, we obtain the smallest whole subscripts:

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At 50ºC:
50 g NH₄Cl----------------- 100 g (H₂O)
? mass NH₄Cl------------- 200 g (H₂O)
mass NH₄Cl = 200 . 50 / 100
mass
It has: 2 atoms of sodium (Na) 1 atom of Carbon 3 atoms of Oxygen bound together with ionic and polar-covalent bonds
Answer:
2 half lives.
Explanation:
Suppose there are 100g of parent isotope at the start.
After 1 half-life there will be 50g of parent and 50g of daughter isotope.
After another half life there is 25 g of parent and 75g of daughter isotope.
You combine 15.00 g of Fe2O3 and 15.00g of CO, which reactant will be limiting