All categories

2 years ago

Which best represents the law of conservation of mass?

Chemistry

2 answers:

disa [49]2 years ago

7 0

Answer:

<h2>D. mass of reactants → mass of products </h2>

Explanation:

The only difference between the options are the sign. The sign between the two is an arrow to represent the change.

(I know this because we're learning about it in class and it's an arrow not an equal, greater, or less than sign)

makkiz [27]2 years ago

6 0

Mass of reactants &gt mass of products

You might be interested in

Which term defines the following: grams of solute divided by 1,000,000 grams of solution

tino4ka555 [31]

The correct answer among the choices is option A. The term that defines the following: grams of solute divided by 1,000,000 grams of solution is called ppm. This is one way of expressing concentration. Parts per million is also equal to 1 milligram of solute per kilogram of solution.

6 0

3 years ago

Read 2 more answers

Which of the following is a inert gas?<br>oxygen<br>chlorine<br>nitrogen<br>aragon

Sophie [7]

Answer:

argon is an inert gas

Explanation:

an inert gas is when a chemical helium, xenon, neon, krypton, radon are also inert gases

5 0

2 years ago

Three glass bulbs, joined by closed stopcocks, have the following volumes and initial pressures of the specified gases.

madam [21]

Answer:

P = 0.75 atm

Explanation:

Using Boyle's law

${P_A}\times {V_A}+{P_B}\times {V_B}+{P_C}\times {V_C}={P}\times {V}$

Given ,

Pressure = 190 torr

The conversion of P(torr) to P(atm) is shown below:

$P(torr)=\frac {1}{760}\times P(atm)$

So,

Pressure = 190 / 760 atm = 0.25 atm

Volume = 200 mL

For Bulb B

Pressure = 1 atm

Volume = 400 mL

For Bulb C

Volume = 1.00 L = 1000 mL

Pressure = 75.994 kPa

The expression for the conversion of pressure in KiloPascal to pressure in atm is shown below:

P (kPa) = $\frac {1}{101.325}$ P (atm)

75.994 kPa = $\frac {75.994}{101.325}$ atm

Pressure = 0.75 atm

Also, Total volume, V = 200 + 400 + 1000 mL = 1600 mL

Using above equation as:

${0.25}\times {200}+{1.00}\times {400}+{0.75}\times {1000}={P}\times {1600}$

We get, Total pressure, P = 0.75 atm

8 0

2 years ago

A gas occupying 2560 ml at 756 mm Hg pressure at standard temperature is transferred to a 4.50 L container , where pressure is 0

posledela

121.2 K

<u>Explanation:</u>

P1V1 / T1 = P2V2 / T2

T2 = P2V2T1 / P1V1

P1, V1, T1, P2, V2 are the known quantities

T2 is the unknown quantity.

Standard temperature, T1 = 273 K

Volume, V1 = 2560 ml is converted to litres as 2.56 L

Pressure, P1 = 756 mm Hg is converted into atm as 0.99 atm

P2 = 0.25 atm and V2 = 4.50 L

Now we have to insert these values in the above equation 2 we will get the temperature, T2 as,

T2 = $\frac{0.25 atm \times 4.50 L \times 273K}{ 0.99 atm \times 2.56 L}$

= 121.2 K

7 0

2 years ago

2C6H5COOH + 15O2 → 14CO2 + 6H2O which of the following options gives the correct product:product ratio? CO2:H2O = 14:6 CO2:H2O =

attashe74 [19]

The products of the reaction are the molecules on the right, thus water and carbon dioxide, hence we eliminate choice 4. Every time the reaction takes place, 14 molecules of CO2 are created and 6 molecules of H2O by the stoicheiometry of the reaction. This ratio will remain throughout the whole reaction, however many reactants are used up. Hence, the correct ratio is CO2:H2O=14:6, answer a).

8 0

3 years ago

Read 2 more answers