All categories

3 years ago

What is the formula mass/molar mass of H2CO2

Chemistry

1 answer:

____ [38]3 years ago

4 0

H - 1.01

C - 12.01

0 - 16.00

2(1.01) + 12.01 + 2(16.00) = 46.03 g/mol

You might be interested in

ASAAAP HURRRY PLS!!!

Setler79 [48]

C or D! When reduced coenzymes produce in the process of the cycle, are oxidized in the process of oxidative phosphorylation in electron transport chain! I hope this helps :(

3 0

3 years ago

Read 2 more answers

Calculate the vapor pressure (in torr) at 298 K in a solution prepared by dissolving 46.8 g of the non-volatile non-electrolye g

Rainbow [258]

<u>Answer:</u> The total partial pressure of the solution is 131.37 torr.

<u>Explanation:</u>

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

<u>For glucose:</u>

Given mass of glucose = 46.8 g

Molar mass of glucose = 180 g/mol

Plugging values in equation 1:

$\text{Moles of glucose}=\frac{46.8g}{180g/mol}=0.26 mol$

<u>For methanol:</u>

Given mass of methanol = 117 g

Molar mass of methanol = 32 g/mol

Plugging values in equation 1:

$\text{Moles of methanol}=\frac{117g}{32g/mol}=3.66 mol$

Mole fraction is defined as the moles of a component present in the total moles of a solution. It is given by the equation:

$\chi_A=\frac{n_A}{n_A+n_B}$ .....(2)

where n is the number of moles

Putting values in equation 2:

$\chi_{methanol}=\frac{3.66}{0.26+3.66}=0.934$

Raoult's law is the law used to calculate the partial pressure of the individual gases present in the mixture. The equation for Raoult's law follows:

$p_A=\chi_A\times p_T$ .....(3)

where $p_A$ is the partial pressure of component A in the mixture and $p_T$ is the total partial pressure of the mixture

We are given:

$p_{methanol}=122.7torr\\\chi_{methanol}=0.934$

Putting values in equation 3, we get:

$122.7torr=0.066\times p_T\\\\p_T=\frac{122.7torr}{0.934}=131.37torr$

Hence, the total partial pressure of the solution is 131.37 torr.

3 0

3 years ago

An element is:

SIZIF [17.4K]

C. A pure chemical substance consisting of one type of atom

3 0

3 years ago

Atmospheric pressure yesterday was given as 0.875 atm. Express this pressure in units of torr and also in kilopascals (kPa), res

Aneli [31]

This problem is about conversion and dimensional analysis. Important information to know:
1 atm = 760 torr = 101.325 kPa

For atm to torr conversion:

0.875 atm * (760 torr / 1 atm) = 665 torr

For atm to kPa conversion:

0.875 atm * (101.325 kPa / atm) = 88.7 kPa

Thus the answer is b) 665 torr and 88.7 kPa

5 0

3 years ago

exactly 1mol of n2o4 is placed in an empty 1 l container. if at equilibrium n2o4 is dissociated 20%, what is the value of equili

egoroff_w [7]

Answer:

K = 0.2

Explanation:

Based on the chemical dissociation of N₂O₄:

N₂O₄ ⇄ 2NO₂

The equilibrium constant, K, of the reaction is:

K = [NO₂]² / [N₂O₄]

Now, if 20% of N₂O₄ is dissociated, 80% remains as N₂O₄ = 0.8mol/L = 0.8M

as 20% is dissociated, 0.2moles of N₂O₄ were dissociated and 0.2*2 = 0.4mol/L of NO₂ are produced.

Replacing in K:

K = [0.4M]² / [0.8M]

5 0

3 years ago