Please Be Honest Rate 1-10

sdas [7]

Answer: alr, gimme a sec

6 0

3 years ago

A student is preparing to perform a series of calorimetry experiments. She first wishes to determine the calorimeter constant (C

Maru [420]

Explanation:

The given data is as follows.

$V_{1}$ = 50 ml, $T_{1}$ = 345 K

$T_{2}$ = 298 K, $T_{f}$ = 317 K,

$V_{2}$ = 50 ml

Now, we will calculate the heat energy as follows.

$Q_{hot} = m \times C_{p} \times (T_{1} - T_{f})$

= $50 g \times 4.184 \times (345 - 317)$

= 5857.6 J

$Q_{cold} = m \times C_{p} \times (T_{f} - T_{2})$

= $50 g \times 4.184 \times (317 - 298)$

= 3974.8 J

As, $Q_{hot} = -Q_{cold}$ so there will be loss of heat. And, some heat will go to the calorimeter.

Hence, $Q_{hot} = Q_{cold} + Q_{cal}$

$5857.6 = 3974.8 + Q_{cal}$

$Q_{cal}$ = 1882.8 J

We assume that the temperature of (calorimeter + water) is 298 K. Hence,

dT = $T_{f} - T_{2}$

= (317 - 298) K

= 19 K

Hence, we will calculate the specific heat as follows.

C = $\frac{Q}{dT}$

= $\frac{1882.8 J}{19}$

= 99.1 J/K

Thus, we can conclude that the value of $C_{cal}$ for the calorimeter is 99.1 J/K.

3 0

4 years ago

TIMED TEST PLEASE HURRY!!! The development of a new experimental method is most likely to change a theory if it makes it possibl

uysha [10]

Answer:

1. analyze the samples while they are frozen

stuff can react differently when it's colder

hope I could help good luck

5 0

3 years ago

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A 8.06 g piece of solid CO 2 is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 300.0 K. What is t

natka813 [3]

Answer:

The pressure of the gas is 4.428 atm.

Explanation:

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

Considering a certain amount of ideal gas confined in a container where the pressure, volume and temperature can vary, but keeping the mass constant, that is, without altering the number of moles, the pressure, P, the temperature can be related, T and the volume, V, of an ideal gas using the ideal gas law:

P*V = n*R*T

where R is the ideal gas constant, and n is the number of moles of the gas.

In this case, to know n you must know the molar mass of the CO₂ compound. Being:

C: 12 g/mole
O: 16 g/mole

then, the molar mass of CO₂ is: 12 g/mole + 2*16 g/mole= 44 g/mole

Then you apply a rule of three: if 44 grams of CO₂ are present in 1 mole, 8.06 grams in how many moles are they?

$moles of CO_{2} =\frac{8.06 grams*1 mole}{44 grams}$

moles of CO₂= 0.18 moles

Then, you know:

P: ?
V: 1 L
n: 0.18 moles

R= 0.082 $\frac{atm*L}{mol*K}$

T= 300 K

Replacing in the equation of the ideal gas law:

P* 1 L= 0.18 moles* 0.082 $\frac{atm*L}{mol*K}$ * 300 K

Solving:

$P=\frac{0.18 moles* 0.082 \frac{atm*L}{mol*K} *300 K}{1 L}$

P= 4.428 atm

The pressure of the gas is 4.428 atm.

3 0

3 years ago

PH is the a measure of the

wlad13 [49]

PH is the measure of concentration of OH- in the solution

6 0

3 years ago

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