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3 years ago

How many grams of CO2 are in 2.1 mol of the compound?

Chemistry

2 answers:

Komok [63]3 years ago

6 0

the awnser is d hope i helped

lawyer [7]3 years ago

3 0

The molar mass of a substance is the mass of one mole of that substance. Therefore, in order to calculate the mass that is present while the number of moles are known, we simply multiply the number of moles present by the molar mass. In the case of carbon dioxide, the molar mass is obtained by adding the mass of one carbon atom (12) and two oxygen atoms (32). The molar mass is 12 + 32 = 44. Therefore, the mass of carbon dioxide is 2.1 * 44 = 92.4 grams. The answer is D.

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Use the portion of the periodic table shown below to answer the questions.

Basile [38]

Part 1: Potassium, and Rubidium.
Part 2: Calcium has 20 protons and 20 electrons because the atomic number for calcium is 20 and that determines how many protons there are and in an atom, the number of protons is the same number of electrons. Calcium has about 20 neutrons. I got the number of Neutrons by subtracting the mass number(40.078) and the atomic number(20), I got 20.078. Round to the nearest whole number because you cannot have half or partial neutron. So, Calcium has 20 protons, 20 electrons, and 20 neutrons,

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8 0

3 years ago

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25 °C = ________ K which one 298 0 33 197

Paraphin [41]

Answer:

298

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Explanation:

5 0

2 years ago

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In which of these statements are protons, electrons, and neutrons correctly compared?

Goryan [66]

the second statement is the correct one quarks are needed to balance charges in all subatomic particles such as neutrons, protons and electrons

3 0

2 years ago

A compound is determined to have the empirical formula C2OH4. If the molar mass of the compound is 132 g/mol, determine the mole

8_murik_8 [283]

Answer: The molecular formula will be $C_6O_3H_{12}$

Explanation:

Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.

Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.

Empirical weight of $C_2OH_{4}$ is $12\times 2+16\times 1+1\times 4=44g$

Molecular mass of compound is = 132 g

Now we have to calculate the molecular formula.

$n=\frac{\text{Molecular weight}}{\text{Equivalent weight}}=\frac{132}{44}=3$

The molecular formula will be= $3\times C_2OH_4=C_6O_3H_{12}$

5 0

2 years ago

55 L of a gas at 25oC has its temperature increased to 35oC. What is its new volume?

ladessa [460]

Answer:

Approximately 56.8 liters.

Assumption: this gas is an ideal gas, and this change in temperature is an isobaric process.

Explanation:

Assume that the gas here acts like an ideal gas. Assume that this process is isobaric (in other words, pressure on the gas stays the same.) By Charles's Law, the volume of an ideal gas is proportional to its absolute temperature when its pressure is constant. In other words

$\displaystyle V_2 = V_1\cdot \frac{T_2}{T_1}$ ,