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3 years ago

What is the proper value for D in the above table. A. 65 B. 35 C. 30 D. 63

Chemistry

2 answers:

tankabanditka [31]3 years ago

8 0

It’s A or C but I think A so just go with A

Zolol [24]3 years ago

5 0

Answer:

Explanation:

Atomic Number, Protons, and Neutrons are always of the same amount.

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If you had a mixture that was found to contain 1.05g SiO2, 0.69g Cellulose and 1.82g Calcium Carbonate. What percentage calcium

boyakko [2]

Percentage by mass = (mass of substance / total mass) x 100
= 1.82 / (1.05 + 0.69 + 1.82) x 100
= 51.1% if Calcium Carbonate

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3 years ago

Formula for the compound Tetraoxygen nonabromide?

Vikentia [17]

Answer:

O4Br9

Explanation:

Tetra means 4 and nona means 9. Just use these prefixes to decide how many of each element you have.

3 0

3 years ago

What is the net ionic equation for AgNO3 and Na2CO3

natima [27]

2Ag+(aq) + CO2-_3(aq)-----------Ag2CO3

5 0

3 years ago

An "empty" container is not really empty if it contains air. How may moles of nitrogen are in an "empty" two-liter cola bottle a

Lisa [10]

Answer:

1. 0.0637 moles of nitrogen.

2. The partial pressure of oxygen is 0.21 atm.

Explanation:

1. If we assume ideal behaviour, we can use the Law of ideal gases to find the moles of nitrogen, considering that air composition is mainly nitrogen (78%), oxygen (21%) and argon (1%):

$V_{N_2}=V_{T}\times 0.78=2L \times 0.78 =1.56 L\\PV=nRT\\n_{N_2}=\frac{PV}{RT}=\frac{1 atm\times 1.56 L}{0.0821\frac{atmL}{molK}\times 298 K}\\n_{N_2}= 0.0637 mol$

2. Now, in order to find he partial pressure of oxygen we need to find the total moles of air, and then the moles of oxygen. Then, we use these results to determine the molar fraction of oxygen, to multiply it with total pressure and get the partial pressure of oxygen as follows:

$n_{total}=\frac{1 atm \times 2L}{0.0821 \frac{atmL}{molK}298K}=0.0817 mol$

$V_{O_2}=2L \times 0.21 = 0.42 L\\n_{O_2}=\frac {1atm \times 0.42 L}{0.0821 \frac{atm L}{mol K}298 K}=0.0172 mol\\X_{O_2}=\frac{n_{O_2}}{n_{total}}=\frac{0.0172 mol}{0.0817 mol}= 0.21$

$P_{O_2}=X_{O_2} \times P = 1 atm \times 0.21 = 0.21 atm$

As you see, the molar fraction and volume fraction are the same because of the assumption of ideal behaviour.

3 0

3 years ago

Please help with these questions ASAP will give brainlist!! CHEMISTRY

Irina18 [472]

Answer:

Question 1 is 21.0g

Explanation:

50 x 4.18 x 3.1 / 0.444 / 69.6= 21.0

4 0

3 years ago