What is the chemical formula for the binary compound composed of au3+ and i- ions?

The tendency of an object to remain at rest or to continue in motion with constant speed in a straight line is called _____.

Ket [755]

Answer:

Inertia

Explanation:

8 0

3 years ago

Need help !!!!! Stuck asap

Step2247 [10]

<h2>Hello!</h2>

The answer is:

Hence, the new pressure will be 2.07 atm.

$P_{2}=2.07atm$

Since we know that the gas is inside of a rigid container, meaning that the volume will be kept constant, we can solve the problem using the Gay-Lussac's Law.

The the Gay-Lussac's Law establishes that when an ideal gas is kept at the same volume, the pressure and the temperature will be proportional.

We need to pay special attention when we are working with the Gay-Lussac's Law since its equaitons works with absolute temperatures (Kelvin ), so, if we are working with relative temperatures such as Celsius degrees or Fahrenheit degrees, we need to convert the temperatures to Kelvin.

We can convert from Celsius degrees to Kelvin using the following formula:

$Temperature(K)=Temperature(C\°)+273$

So, we have the Gay-Lussac's equation:

$\frac{P_{1}}{T_{1}}=\frac{P_{2}}{T_{2}}$

Also, we are given the following information:

$T_{1}=30\° \\P_{1}=2atm\\T_{2}=40\°$

Therefore, converting the temperature to Kelvin, we have:

$T_{1}=30C\°=30+273K=303K\\\\T_{1}=40C\°=40+273K=313K\\$

Now, calculating we have:

$\frac{P_{1}}{T_{1}}=\frac{P_{2}}{T_{2}}$

$P_{2}=\frac{P_{1}}{T_{1}}*T_{2}\\\\P_{2}=\frac{2atm}{303K}*313K=2.07atm$

Hence, the new pressure will be 2.07 atm.

$P_{2}=2.07atm$

Have a nice day!

4 0

4 years ago

A bowl containing 70 grams of water, is heated from 10 °C to 90 °C. The specific heat of

storchak [24]

Answer:

23430.4 J.

Explanation:

From the question given above, the following data were obtained:

Mass (M) = 70 g

Initial temperature (T₁) = 10 °C

Final temperature (T₂) = 90 °C

Specific heat capacity (C) = 4.184 J/gºC

Heat (Q) required =?

Next, we shall determine the change in the temperature of water. This can be obtained as follow:

Initial temperature (T₁) = 10 °C

Final temperature (T₂) = 90 °C

Change in temperature (ΔT) =?

ΔT = T₂ – T₁

ΔT = 90 – 10

ΔT = 80 °C

Finally, we shall determine the heat energy required to heat up the water. This can be obtained as follow:

Mass (M) = 70 g

Change in temperature (ΔT) = 80 °C

Specific heat capacity (C) = 4.184 J/gºC

Heat (Q) required =?

Q = MCΔT

Q = 70 × 4.184 × 80

Q = 23430.4 J

Therefore, 23430.4 J of heat energy is required to heat up the water.

4 0

3 years ago

When a reaction forms between atoms with ground state electron configuration 1s22s2 and 1s22s22p5 the predominant type of bond f

Arisa [49]

C. Ionic is the answer

6 0

3 years ago

b) 2C2H2(g) + 5O2(g)⟶4CO2(g) + 2H2O(l) 6.54 Calculate the heats of combustion for the following reactions from the standard enth

IRINA_888 [86]

Answer:

a. ΔH⁸ = -1420 kJ/mol b. ΔH⁸ = -1144.84 kJ/mol

Explanation:

a.

C₂H₄ (g) + 3 O₂ (g) ------------------------ 4 CO₂ (g) + 2 H₂O (l) ΔH⁸ = ?

ΔH⁸f kJmol 52.47 0 -399.5 -285.83

ΔH⁸ = 2(-399.5) + 2 (-285.83) - (52.47)

ΔH⁸ = -1420 kJ/mol

b.

H₂S (g) + 3 O₂ (g) ---------------------- 2 H₂O (l) + 2 SO₂ (g)

ΔH⁸f kJmol -20.50 0 -285.83 -296.84

ΔH⁸ = 2(-285.83) + 2 (-296.84) - (-20.50)

ΔH⁸ = -1144.84 kJ/mol

4 0

3 years ago