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3 years ago

Formula for tin (II) sulfide

Chemistry

2 answers:

irakobra [83]3 years ago

5 0

Answer:

SnS

Explanation:

Tin, as it shows on the periodic table can have a +2 or +4 charge.

Sulfide is just Sulfur which has a -2 charge.

It tells us the charge of the tin in roman numerals. In this case (II) means two, so it is tin with a charge of two.

In order for these to balance each other, we are going to take one of the tin and one of the sulfur because it the +2 and -2 add to zero.

igor_vitrenko [27]3 years ago

4 0

Answer:

SnS

Explanation:

Tin(II) sulfide is a chemical compound of tin and sulfur. The chemical formula is SnS. Its natural occurrence concerns herzenbergite, a rare mineral.

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Svetlanka [38]

The temperature of the countertop changes by 0.032 °C

The quantity of heat transferred to the countertop is given by

Q = CΔT where Q = quantity of heat transferred to the countertop = 5000 J = 5 kJ, C = heat capacity of the countertop = 158.5 kJ/°C and ΔT = temperature change of the countertop.

Since we require the temperature change of the countertop, we make ΔT subject of the formula.

So, ΔT = Q/C

So, substituting the values of the variables into the equation, we have

ΔT = Q/C

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ΔT = 0.032 °C

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3 years ago

What is the mass in 0.25 mol of SO2

gulaghasi [49]

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3 years ago

The hydrogen bonding in water creates ________, a cohesive force that enables one to slightly overfill a glass with water or all

ziro4ka [17]

Answer: -

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3 years ago

How many milligrams of magnesium reacts with excess HCl to produce 31.2 mL of hydrogen gas at 754 Torr and 25.0℃.

Ivanshal [37]

Answer:

There will react 30.9 milligrams of magnesium

Explanation:

Step 1: Data given

Volume of hydrogen = 31.2 mL

Pressure = 754 torr = 754/760 = 0.992 atm

Temperature = 25.0 °C = 298 Kelvin

Step 2: The balanced equation

Mg + 2HCl → MgCl2 + H2

Step 3: Calculate moles of H2

p*V = n*R*T

⇒ with p = the pressure of H2 = 0.992 atm

⇒with V = the volume of H2 = 31.2 mL = 0.0312 L

⇒ with n = the moles of H2 = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T= the temperature = 25.0 °C = 298 Kelvin

n = (p*V)/(R*T)

n = (0.992*0.0312)/(0.08206*298)

n = 0.00127 moles

Step 4: Calculate moles of Mg

For 1 mol of Mg we need 2 moles of HCl to produce 1 mol of MgCl2 and 1 mol of H2

For 0.00127 moles of H2 we need 0.00127 moles of Mg

Step 5: Calculate mass of Mg

Mass of Mg = moles of Mg * molar mass of Mg

Mass of Mg = 0.00127 moles * 24.3 g/mol

Mass of Mg = 0.0309 grams = 30.9 mg of Mg

There will react 30.9 milligrams of magnesium

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2 years ago