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4 years ago

Who was the first chemist to perform truly quantitative experiments?

1 answer:

3 0

Chemistry II, Zumdahl 7th edit, Chapter#2 Questions Bank
A B
The first chemist to perform truly quantitative experiments was? Robert Boyle
The scientist whom discovered the Law of Conservation of Mass is also called the Father of Modern chemistry.Who is that scientist?

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2H2+O2-->2H2O, If you have 9 moles of Hydrogen gas (H2), how many moles of water can you form? (Enter just the number: not th

Naddika [18.5K]

If you have 9 moles of hydrogen gas(H2) the moles of water that can be formed is 9 moles

calculation

2H2 +O2→ 2H2O

The mole of H2O is calculated using the mole ratio.

that is H2:H2O is 2:2 into simple form = 1:1

therefore if 9 moles of H2 reacted the moles of H2O = 9 x1/1 = 9 moles

8 0

3 years ago

Part A What benefit does figure 1 have over the other visualizations?

Mars2501 [29]

Answer:

Figure 1 provides the rawest and most accurate data.

Explanation:

8 0

3 years ago

A 150 W electric heater operates for 12.0 min to heat an ideal gas in a cylinder. During this time, the gas expands from 3.00 L

Brut [27]

Answer: The change in internal energy of the gas is 108.835 kJ

Explanation:

To calculate the work done for reversible expansion process, we use the equation:

$W=P\Delta V=-P(V_2-V_1)$

where,

W = work done

P = pressure = 1.03 atm

$V_1$ = initial volume = 3.00 L

$V_2$ = final volume = 11.0 L

Putting values in above equation, we get:

$W=-(1.03)\times (11.0-3.00)=8.24L.atm=834.9J=0.835kJ$ (Conversion factor: 1 L. atm = 101.325 J)

Calculating the heat from power:

$Q=P\times t$

where,

Q = heat required

P = power = 150 W

t = time = 12 min = 720 s (Conversion factor: 1 min = 60 s)

Putting values in above equation:

$Q=150\times 720=108000J=108kJ$

The equation for first law of thermodynamics follows:

$Q=dU+W$

where,

Q = total amount of heat required = 108 kJ

dU = Change in internal energy = ?

W = work done = -0.835 kJ

Putting values in above equation, we get:

$108kJ=dU+(-0.835)\\\\dU=(108+0.835)=108.835kJ$

Hence, the change in internal energy of the gas is 108.835 kJ

7 0

4 years ago

the buret is dirty and drops of NaOH cling to the side walls of the buret as it drained. How does this affect the result for NaO

kykrilka [37]

Since this has to do with titration, the measured volume of NaOH used would be less than the actual volume used because some of the unused NaOH would cling to the sides of the buret and therefore wouldn't factor into the measurement

Hope this helps

6 0

4 years ago

If I have 9 moles of a gas at a pressure of 8.7 atm and a volume of 18 liters, what is the temperature?

alukav5142 [94]

212K
pV=nRT.
R = 0.08206

5 0

4 years ago