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Mrrafil [7]
3 years ago
15

How to calculate percentage change in mass

Chemistry
1 answer:
blondinia [14]3 years ago
3 0
In order to find the percentage change in mass, you must d<span>ivide </span>Change in Mass<span> by Initial </span>Mass<span>. After that, you divide the </span>change in mass<span> by the initial </span>mass<span> of your substance.

   This calculation shows what proportion of the initial </span>mass<span> changed. To find the </span>percent change<span>, simply multiply this number by 100</span>
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What weight of sodium hydroxide will react with 73 gram of hydrogen chloride gas at NTP to Produce 117.0 gram of Nacl and 36 gra
Wewaii [24]

Let's write the equation

\\ \sf\longmapsto {NaOH\atop ?}+{HCl\atop 73g}\longrightarrow {NaCl\atop 117g}+{H_2O\atop 36g}

According to law of conservation of mass .

  • Mass of products=Mass of reactants

Let required value be x

\\ \sf\longmapsto x+73=117+36

\\ \sf\longmapsto x+73=153

\\ \sf\longmapsto x=153-73

\\ \sf\longmapsto x=80g

8 0
2 years ago
Read 2 more answers
How many moles are contained in 2.0 L of N2 at standard temperature and pressure.
GuDViN [60]

0.091 moles are contained in 2.0 L of N2 at standard temperature and pressure.

Explanation:

Data given:

volume of the nitrogen gas = 2 litres

Standard temperature = 273 K

Standard pressure = 1 atm

number of moles =?

R (gas constant) = 0.08201 L atm/mole K

Assuming nitrogen to be an ideal gas at STP, we will use Ideal Gas law

PV = nRT

rearranging the  equation to calculate number of moles:

PV = nRT

n = \frac{PV}{RT}

putting the values in the equation:

n = \frac{1X2}{0.08201 X 273}

n = 0.091 moles

0.091 moles of nitrogen gas is contained in a container at STP.

6 0
3 years ago
A gas expands from a volume of 2.00L at 36.0oC to a volume of 2.50 L, what is the final temperature, if the pressure is constant
lakkis [162]
We shall consider V, the volume and T, the temperature.
According to Boyle's Laws:
\frac{V1}{T1} = \frac{V2}{T2}
In our case:
\frac{2.00}{36.0} = \frac{2.50}{T2} =\ \textgreater \  T2= \frac{2.50*36.00}{2.00} = 45
6 0
3 years ago
Read 2 more answers
When copper metal is added to nitric acid, the following reaction takes place
zlopas [31]

Answer:

The volume of NO₂ gas collected over water at 25.0 °C is 1.68 Liters.

Explanation:

Cu (s) + 4 HNO_3 (aq) \rightarrow Cu(NO_3)_2 (aq) + 2 H_2O (l) + 2 NO_2 (g)

Moles of copper = \frac{2.01 g}{63.55 g/mol}=0.03163 mol

According to reaction, 1 mol of copper gives 2 moles of nitrogen dioxide gas.

Then 0.03613 moles of copper will give:

\frac{2}{1}\times 0.03163 mol=0.06326 mol of nitrogen dioxide gas

Moles of nitrogen dioxide gas = n = 0.06326 mol

Pressure of the gas = P

P = Total pressure - vapor pressure of water

P = 726 mmHg - 23.8 mmHg = 702.2 mmHg

P = 0.924 atm (1 atm = 760 mmHg)

Temperature of the gas = T = 25.0°C =298.15 K

Volume of the gas = V

PV=nRT

V=\frac{0.06326 mol\times 0.0821 atm L/mol K\times 298.15 K}{0.924 atm}

V = 1.68 L

The volume of NO₂ gas collected over water at 25.0 °C is 1.68 Liters.

3 0
3 years ago
This group of elements contains brittle solids at room temperature. They
Natalija [7]

non-metals

they don't conduct heat

5 0
3 years ago
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