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3 years ago

Can someone help? This question is very difficult for me

Chemistry

1 answer:

stich3 [128]3 years ago

3 0

<h3>Solution:</h3>

According to law of conservation of matter, mass of reactants = mass of product formed.
Here, mass of hydrogen = 30 grams
Mass of oxygen = 30 grams
Hydrogen + Oxygen = Dihydrogen monoxide
Therefore, Mass of hydrogen + Mass of oxygen = Mass of Dihydrogen Monoxide
So, 30 grams + 30 grams = 60 grams.
So, 60 grams of dihydrogen monoxide is present in the product.

<h3>Answer:</h3>

A. 60 grams

Hope it helps

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what is the empirical formula for a substance if a 1.000 g sample of it contains 0.262 grams of nitrogen, 0.075 grams of hydroge

Sonbull [250]

Here are the steps for finding an emprical formula.

To begin, we need to change the grams to a percentage. We can simply take the number and call it our percentage. (i.e 0.262%)

Then, we have a simply stoichiometry step. We put our starting number over 1, as usual. The next "Step" is putting in the molar mass of that particular element on the bottom, with one on top. It should look like this:

0.262% N 1
-------------- x ----------------
1 14.007g N

We would then divide those two numbers to get our answer. Repeat for the other elements included, until we have all of them done.

After that, we need to find the smallest number that was the answer to one of the equations. For example, if the product of Hydrogen was the smallest formed, we would locate that number. We then divide ALL of our answers by that smallest number.

Remember, whenever doing empirical formulas, significant figures matter.

Once we have our smallest numbers, we need to round our numbers to the nearest whole number. HOWEVER, to do this we need to multiply all of the numbers by the SAME whole number.

For example, if one of our numbers was 1.33, we would multiply by 3 to get a whole number. However, we would also need to multiply the rest of our products by the same number. If we do not get close to whole numbers (you can round), we need to try with multiplying a different number.

Then, we need to take those whole numbers we got for each number, and plug in to make a compound. For example, if our products were 6 for nitrogen, 3 for hydrogen, and 2 for chlorine, our final empirical formula would be N6H3Cl2.

Hope I could help! If it was a bit wordy please let me know and I'd be more than willing to clarify.

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3 years ago

A sample of gas has a mass of 0.673g. Its volume is 250.0mL at a temperature of 83 degrees C and a pressure of 747 torr. The sam

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Answer:

Explanation:

Given data:

Mass of sample = 0.673 g

Volume = 250.0 mL (0.25 L)

Temperature = 83°C (273+83= 356 k)

Pressure = 747 torr (747/760 = 0.98 atm)

Gas type = ?

Solution:

PV = nRT

n = PV/RT

n = 0.98 atm× 0.25 L / 0.0821 atm. L/mol.K × 356 k

n = 0.245 / 29.23/mol

n = 0.01 mol

Number of moles = mass/ molar mass

Molar mass = 0.673 g / 0.01 mol

Molar mass = 67.3 g/mol

molar mass of CO2 = 44 g/mol

molar mass of H2 = 2.016 g/mol

molar mass of SO3 = 80.066 g/mol

molar mass of Ar = 40 g/mol

molar mass of Xe = 131.3 g/mol

So non of these gases are present.

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4 years ago

Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M.Express your answer to two significant f

N76 [4]

The question is incomplete, here is the complete question:

Calculate the initial rate for the formation of C at 25°C, if [A]=0.50 M and [B]=0.075 M. Express your answer to two significant figures and include the appropriate units.Consider the reaction

A + 2B ⇔ C

whose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table:

The table is attached below as an image.

<u>Answer:</u> The initial rate for the formation of C at 25°C is $2.25\times 10^{-2}Ms^{-1}$

<u>Explanation:</u>

Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

For the given chemical equation:

$A+2B\rightleftharpoons C$