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puteri [66]
3 years ago
5

What about 50 g of water? I need help what this

Chemistry
1 answer:
ELEN [110]3 years ago
3 0

Answer:

3.38  Tablespoons

10.14 Teaspoons

0.21 U.S. Cups

0.18 Imperial Cups

0.20 Metric Cups

50.00 Milliliters

Explanation:

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Tin(II) fluoride (SnF2) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of F in grams in
Alexeev081 [22]

Answer:

In 33.7 grams SnF2 we have 8.17 grams of F

Explanation:

Step 1: Data given

Mass of SnF2 = 33.7 grams

Molar mass of SnF2 = 156.69 g/mol

Molar mass of F = 19.00 g/mol

Step 2: Calculate moles of SnF2

Moles SnF2 = mass / molar mass

Moles SnF2 = 33.7 grams / 156.69 g/mol

Moles SnF2 = 0.215 moles

Step 3: Calculate moles F

For 1 mol SnF2 we have 2 moles F

For 0.215 moles SnF2 we have 2*0.215 = 0.430 moles F

Step 4: Calculate mass F

Mass F = moles F * molar mass F

Mass F = 0.430 moles * 19.00 g/mol

Mass F = 8.17 grams

In 33.7 grams SnF2 we have 8.17 grams of F

6 0
3 years ago
Pentaborane-9, B5H9, is a colorless, highly reactive liquid that will burst into flame when exposed to oxygen. The reaction is 2
mina [271]

<u>Answer:</u> The amount of energy released per gram of B_5H_9 is -71.92 kJ

<u>Explanation:</u>

For the given chemical reaction:

2B_5H_9(l)+12O_2(g)\rightarrow 5B_2O_3(s)+9H_2O(l)

The equation used to calculate enthalpy change is of a reaction is:  

\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f_{(product)}]-\sum [n\times \Delta H^o_f_{(reactant)}]

The equation for the enthalpy change of the above reaction is:

\Delta H^o_{rxn}=[(5\times \Delta H^o_f_{(B_2O_3(s))})+(9\times \Delta H^o_f_{(H_2O(l))})]-[(2\times \Delta H^o_f_{(B_5H_9(l))})+(12\times \Delta H^o_f_{(O_2(g))})]

Taking the standard enthalpy of formation:

\Delta H^o_f_{(B_2O_3(s))}=-1271.94kJ/mol\\\Delta H^o_f_{(H_2O(l))}=-285.83kJ/mol\\\Delta H^o_f_{(B_5H_9(l))}=73.2kJ/mol\\\Delta H^o_f_{(O_2(g))}=0kJ/mol

Putting values in above equation, we get:

\Delta H^o_{rxn}=[(5\times (1271.94))+(9\times (-285.83))]-[(2\times (73.2))+(12\times (0))]\\\\\Delta H^o_{rxn}=-9078.57kJ

We know that:

Molar mass of pentaborane -9 = 63.12 g/mol

By Stoichiometry of the reaction:

If 2 moles of B_5H_9 produces -9078.57 kJ of energy.

Or,

If (2\times 63.12)g of B_5H_9 produces -9078.57 kJ of energy

Then, 1 gram of B_5H_9 will produce = \frac{-9078.57kJ}{(2\times 63.12)}\times 1g=-71.92kJ of energy.

Hence, the amount of energy released per gram of B_5H_9 is -71.92 kJ

8 0
3 years ago
The horse achieved its highest status during the___________dynasty (618-906 CE), a time of unparalleled political, artist, and c
inessss [21]
The answer is c i hopenit helps:)
3 0
3 years ago
Consider the following reaction: . SO2Cl2(g)⇌SO2(g)+Cl2(g) . A reaction mixture is made containing an initial [SO2Cl2] of 2.2×10
Alex Ar [27]
The equilibrium constant (Kc) is the product of the equilibrium concentrations of the products raised to their corresponding stoichiometric coefficients divided by the reactants as well. In this case the equilibrium concentration of Cl2 which also applies to SO2 is 1.3x10^-2. The final equilibrium concentration of SO2Cl2 is 9x10^-3. Kc is then equal to 0.0188.
3 0
3 years ago
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Nonmetal halogen family atmoic mass 35
Anettt [7]

chlorine has the atomic mass of 35.5 and is a non metal in the halogen family

5 0
3 years ago
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