Which compound has the highest melting point? Picture has the options

Hydrazine reacts with oxygen according to the following equation: N2H4(g) +O2(g) → N2(g) + 2 H2O(l) How many L of N2, measured a

mihalych1998 [28]

Answer:

V ≈ 646.50 L

General Formulas and Concepts:

Chemistry - Gas Laws

Reading a Periodic Table
Stoichiometry
Combined Gas Law: PV = nRT
R constant - 62.4 (L · torr)/(mol · K)
Kelvin Conversion: K = °C + 273.15

Explanation:

Step 1: Define

RxN: N₂H₄ (g) + O₂ (g) → N₂ (g) + 2H₂O (l)

Given: 34.9 °C, 755.08 torr, 914.894 g H₂O

Step 2: Identify Conversions

Kelvin Conversion

Molar Mass of H - 1.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol

Step 3: Convert

Stoichiometry: $914.894 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O} )(\frac{1 \ mol \ N_2}{2 \ mol \ H_2O} )$ = 25.3955 mol N₂

Temperature: 34.9 + 273.15 = 308.05 K

Step 4: Find Volume

Substitute variables: (755.08 torr)V = (25.3955 mol)(62.4 (L · torr)/(mol · K))(308.05 K)
Multiply: (755.08 torr)V = 488160 L · torr
Isolate V: V = 646.502 L

Step 5: Check

We are given 5 sig figs as our lowest. Follow sig fig rules and round.

646.502 L ≈ 646.50 L

6 0

3 years ago

Which formation is one feature of karst topography?

Aleksandr [31]

The answer is caves.. i think

6 0

3 years ago

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Why must sample spots be above the solvent in paper chromatography

marishachu [46]

Because if they are submerged in the solvent, they would dissolve! This would prevent them from seperating and not allow you to actually record anything

6 0

3 years ago

How do i solve number 36?

tresset_1 [31]

To cut this short and for your understanding, ionic bond is formed between metals (mostly right column in periodic table). Covalent bond is formed between non-metals (mostly left column in periodic table). So polar covalent is also a covalent bond but it is polar, which means the shape of molecules are not symmetrical hence maybe an atom in a molecule has most of the electron attracted to it causing itself to be partial negative (since electron are negatively charged) and the other atom has its electron being attracted by others became partial positive. Polar covalent can also be when H atom is binding either to F, O or N (also known as hydrogen bond).

6 0

3 years ago

What mass of butane in grams is necessary to produce 1.5×103 kj of heat what mass of co2 is produced?

kari74 [83]

The heat of reaction (i.e. combustion) of butane ( $C_{4} H_{10}$ ) when reacted with oxygen ( $O_{2}$ )  is -2658 kJ/mol butane, and the chemical reaction is given by:

$C_{4} H_{10}$ + $\frac{13}{2} O_{2}$ ---> $4 CO_{2}$ + $5 H_{2}O$

The mass of butane required in the reaction is based on the heat produced by the reaction, which is given to be -1,500 kJ. The minus sign is added because the reaction releases heat (exothermic), which means that the products are in a "lower energy state" than the reactants.

Dividing this with the heat of reaction per mole of butane reacted would give the number of moles butane required. Then, multiplying the answer with the molar mass of butane which is 58 grams/mole, will give the mass of butane required.

Moles of butane = [(-1,500 kJ)/(-2658 kJ/mol butane)]
Moles of butane = 0.5643 moles butane

Mass of butane  = 0.5643 moles butane * 58 grams/mol butane
Mass of butane = 32.73 grams butane

The mass of carbon dioxide ( $CO_{2}$ ) can be determined by multiplying the moles of butane ( $C_{4} H_{10}$ ) with the mole ratio of ( $CO_{2}$ ) produced to the ( $C_{4} H_{10}$ ) reacted, and then with the molar mass of ( $CO_{2}$ ), which is 44 grams/mole.

Mass of carbon dioxide produced
= 0.5643 moles butane * [4 moles $CO_{2}$ / 1 mole $C_{4} H_{10}$ ] * 44 grams/mole $CO_{2}$

Mass of carbon dioxide produced
= 99.32 grams $CO_{2}$

Thus, the mass of butane required is 32.73 grams, and the mass of carbon dioxide produced from the reaction of this amount of butane is 99.32 grams.

4 0

3 years ago

Read 2 more answers