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Tju [1.3M]
3 years ago
12

What is the mass number of an atom that has 12 neutrons and 11 protons? 24 12 11 23

Chemistry
1 answer:
Gre4nikov [31]3 years ago
5 0

Answer:

23

Explanation:

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If the force is 2,500 N and the acceleration is 500 m/s/s, what is the objects mass
ra1l [238]
The mass is 5kg
I hope this helps
5 0
2 years ago
How many grams of F are in 12.56 g of SF6? h.
natali 33 [55]

Answer:

9.80 g

Explanation:

The molecular mass of the atoms mentioned in the question is as follows -

S = 32 g / mol

F = 19 g / mol

The molecular mass of the compound , SF₆ = 32 + ( 6 * 19 ) = 146 g / mol

The mass of 6 F = 6 * 19 = 114 g /mol .

The percentage of F in the compound =

mass of 6 F / total mass of the compound * 100

Hence ,  

The percentage of F in the compound = 114 g /mol  / 146 g / mol * 100

78.08 %

Hence , from the question ,

In 12.56 g of the compound ,

The grams of F = 0.7808 * 12.56 = 9.80 g

4 0
3 years ago
2. Some nitrogen at a pressure of 35.75 p.s.i is in a 100 L container. If the container's volume is reduced to 2250 ml then what
elena-s [515]

Answer:

1455.6

Explanation: you first convert 2250ml to l by dividing by 1000 so you get 2.25l then you use Boyles law which is p1v1=p2v2 then insert values

35.75*100=p2*2.25 then divide both sides by 2.25 then you get 1455.6

4 0
3 years ago
Hydrogen gas at a pressure of 740. mmHg has a volume of 2.00 L at a temperature of 25.0°C. What is the temperature of this gas a
nikdorinn [45]

Answer:

The final temperature of hydrogen gas is  537.63 K.

Explanation:

Given data:

Initial volume = 2.00 L

Initial pressure = 740 mmHg (740/760 = 0.97 atm)

Initial temperature = 25 °C (25 +273 = 298 K)

Final temperature =?

Final volume = 3.50 L

Final pressure = standard = 1 atm

Formula:  

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

P₁V₁/T₁ = P₂V₂/T₂

T₂  =  P₂V₂T₁  / P₁V₁

T₂ = 1 atm × 3.5 L × 298 K / 0.97 atm × 2.00 L  

T₂ = 1043  atm .L. K / 1.94 atm. L

T₂ = 537.63 K

7 0
3 years ago
Gaseous ammonia chemically reacts with oxygen O2 gas to produce nitrogen monoxide gas and water vapor. Calculate the moles of am
mel-nik [20]

Answer:

1.7 moles of ammonia, NH₃.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

4NH₃ + 5O₂ —> 4NO + 6H₂O

From the balanced equation above,

4 moles of NH₃ reacted to produce 4 moles of NO.

Finally, we shall determine the number of mole of ammonia, NH₃, needed to produce 1.7 moles of nitrogen monoxide, NO. This can be obtained as follow:

From the balanced equation above,

4 moles of NH₃ reacted to produce 4 moles of NO.

Therefore, 1.7 moles of NH₃ will also react to produce 1.7 moles of NO.

Thus, 1.7 moles of ammonia, NH₃, is required.

5 0
2 years ago
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