Response:
of 
can be found in 39.5 grams of .
Clarification:
Atomic weights: P= 31, F= 19,
The molar mass equals 1 atomic weight of P + 5 atomic weights of
F= 31+5 × 19
= 31+95
=126 g/mole
The number of moles in 39.5 gm of
equals 
= 
=0.3134 moles
1 mole of any substance encompasses
0.3131 moles comprises 0.3134
Thus, of can be found in 39.5 grams of .
Answer:
2(CH3)2N2H2 + 3N2O4 → 4N2 + 4H2O + 4CO2 + heat
Explanation:
- To balance chemical equations, coefficients are assigned to both reactants and products.
- This yields an equal count of atoms of each element on both sides of the equation.
- Balancing chemical equations ensures compliance with the law of conservation of mass.
- According to this law, the mass of reactants must equal the mass of products, achievable through balancing the equation.
- The application of coefficients 2, 3, 4, 4, 4 allows for an equal balance in the equation.
- Consequently, the balanced equation can be written as:
2(CH3)2N2H2 + 3N2O4 → 4N2 + 4H2O + 4CO2 + heat
Answer:
The forward reaction will keep occurring until all NO or all NO₂ is consumed.
Clarification:
- According to Le Châtelier's principle, when a system at equilibrium experiences a disturbance from an outside source, the system will adjust to counteract this disturbance and restore equilibrium.
- Thus, removing the product (N₂O₃) from the system effectively lowers the product concentration, prompting the reaction to shift forward and generate additional product in order to alleviate the strain caused by the removal of N₂O₃.
- Consequently, the reaction will proceed forward until all of either NO or NO₂ is depleted.
Explanation:
Initial moles of ethanoic acid = 0.020 mol
At equilibrium, half of the ethanoic acid molecules have reacted.
Thus, moles of ethanoic acid reacted = 0.020 mol * (50% / 100%)
= 0.010 mol
Moles of ethanoic acid remaining = 0.020 mol - 0.010 mol = 0.010 mol
The moles of product 
gas formed are determined as follows:
0.010 mol CH3COOH * (1 mol / 2 mol CH3COOH)
= 0.005 mol
Consequently, the total moles of gas present in the vessel at equilibrium are 0.010 mol CH3COOH and 0.005 mol
Total gas moles at equilibrium = 0.010 mol + 0.005 mol = 0.015 mol
Next, let’s determine the pressure:
0.020 mol of gas has a pressure of 0.74 atm; so under the same conditions, we find the pressure exerted by 0.015 mol of gas:
P1/n1 = P2/n2
P2 = P1*(n2 / n1)
= 0.74 atm * (0.015 mol / 0.020 mol)
= 0.555 atm
Response:
CRYSTAL
A LARGE NUMBER OF ATOMS ORGANIZED IN A REGULAR STRUCTURE
1:1
Reasoning:
